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Heat of Formation

Consider the ...

Question

Consider the following reactions:
(a) $H_{(a q)}^{+} + O H_{(a q)}^{-} = H_{2} O_{(I)}, △ H = - X_{1} k J m o l^{- 1}$
(b) $H_{2 (g)} + \frac{1}{2} O_{2 (g)} = H_{2} O_{(I)}, △ H = - X_{2} k J m o l^{- 1}$
(c) $C O_{2 (g)} + H_{2 (g)} = C O_{(g)} + H_{2} O_{(I)} - X_{3} k J m o l^{- 1}$
(d) $C_{2} H_{2 (g)} + \frac{5}{2} O_{2 (g)} = 2 C O_{2 (g)} + H_{2} O_{(I)} + X_{4} k J m o l^{- 1}$ .
Enthalpy of formation of $H_{2} O_{(l)}$ is:

+ X_{1} k J m o l^{- 1}

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- X_{2} k J m o l^{- 1}

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+ X_{3} k J m o l^{- 1}

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- X_{4} k J m o l^{- 1}

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Solution

The correct option is B $- X_{2} k J m o l^{- 1}$
3-Bromo 2-methyl prop-1-ene

For enthalpy of formation all the constituent molecule should be in standard form

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l)$

$Δ H = - X_{2} k J m o l^{- 1}$

option B is correct option

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Similar questions

Consider the following reactions:

(a) $H^{+} (a q) + O H^{-} (a q) \to H_{2} O (l) Δ H = - x_{1} k J m o l^{- 1}$

(b) $H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l) Δ H = - x_{2} k J m o l^{- 1}$

(d) $C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) \to 2 C O_{2} (g) + H_{2} O (l) Δ H = x_{4} k J m o l^{- 1}$

Enthalpy of formation of $H_{2} O (l)$ is

H_{(a q)}^{+} + O H_{(a q)}^{-} = H_{2} O_{(l)}, Δ H = - X_{1}

m o l^{- 1}

H_{2 (g)} + \frac{1}{2} O_{2 (g)} = H_{2} O_{(l)}, Δ H = X_{2}

m o l^{- 1}

C O_{2 (g)} + H_{2 (g)} = C O_{(g)} + H_{2} O_{(l)} - X_{3}

m o l^{- 1}

C_{2} H_{2 (g)} + \frac{5}{2} O_{2 (g)} = 2 C O_{2 (g)} + H_{2} O_{(l)} + X_{4}

m o l^{- 1}

H_{2} O_{(l)}

C H_{3} O H (1) + \frac{3}{2} O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (I); Δ, H^{⊖} = - 726 k J m o l^{- 1}

C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g); Δ_{c} H^{⊖} = - 393 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (I); Δ_{f} H^{⊖} = - 286 k J m o l^{- 1}

{C H}_{3} O H (l)

H^{+} (a q) + O H^{-} (a q) = H_{2} O (l); Δ H = - X_{1} k J . m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) = H_{2} O (l); Δ H = - X_{2} k J . m o l^{- 1}

C O_{2} (g) + H_{2} (g) = C O (g) + H_{2} O (l); Δ H = + X_{3} k J . m o l^{- 1}

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) = 2 C O (g) + H_{2} O (l); Δ H = + X_{4} k J . m o l^{- 1}

H_{2} O (l)

2 C (s) + 2 O_{2} (g) \to 2 C O_{2} (g)

Δ H = - 787

H_{2} (g) + 1_{/ 2} O_{2} (g) \to H_{2} O (l)

Δ

= - 286

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) \to 2 C O_{2} (g) + H_{2} O (l)

Δ

= - 1310

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